How can electronic transitions in atoms contribute to the vibration of molecules?
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Molecular vibration. A molecular vibration occurs when atoms in amolecule are in periodic motion while the molecule as a whole has constant translational and rotational motion. ... A fundamentalvibration is excited when one such quantum of energy is absorbed by the molecule in its ground state.
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transitions of an electron in a H-atom would emit a photon of minimum wavelength :-
6 to 1 (assuming “1” is ground state and “6” is 6th orbit or 5th exited state of Hydrogen atom)
You don’t have to perform any calculation to answer this multiple choice question. I was able to tell the correct answer and energy of photon in electron volts (ev) for every transition as soon as I saw these options.
You have to find which transition will emit a photon of minimum wavelength. In other words, you have to find a transition which will emit a photon of maximum energy/frequency. (min. wavelength → max. frequency, because speed of photon is constant).
Total energy of an electron in a H-like atom: −13.6 z2/n2 ev
z=atomic number (1 for hydrogen), n=orbit number
For n=1 in Hydrogen, total energy = −13.6ev. (in ground state)
For n=2, it is −3.4ev
Similarly, you can find the energy of every orbit in any hydrogen like atom.
In 6 to 1 transition the energy difference is highest, so the frequency of photon emitted will also be highest, thus, its wavelength will be lowest.
6 to 1 (assuming “1” is ground state and “6” is 6th orbit or 5th exited state of Hydrogen atom)
You don’t have to perform any calculation to answer this multiple choice question. I was able to tell the correct answer and energy of photon in electron volts (ev) for every transition as soon as I saw these options.
You have to find which transition will emit a photon of minimum wavelength. In other words, you have to find a transition which will emit a photon of maximum energy/frequency. (min. wavelength → max. frequency, because speed of photon is constant).
Total energy of an electron in a H-like atom: −13.6 z2/n2 ev
z=atomic number (1 for hydrogen), n=orbit number
For n=1 in Hydrogen, total energy = −13.6ev. (in ground state)
For n=2, it is −3.4ev
Similarly, you can find the energy of every orbit in any hydrogen like atom.
In 6 to 1 transition the energy difference is highest, so the frequency of photon emitted will also be highest, thus, its wavelength will be lowest.
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